What will be the pH of `0.05`M barium hydroxide solution ?

Options

A. `8`
B. `9`
C. `7`
D. `13`

Explanation

Barium hydroxide is a strong electrolyte, i.e., it dissociates completely:
`Ba(OH)_(2)(aq.)rarr Ba^(2+)(aq.)+2OH^(-)(aq.)`
According to the equation,
`C_(OH^(-))=2C_(Ba(OH)_(2))=(2xx0.05)M`
`=0.1M`
`=10^(-1)M`
`:. C_(OH^(-))= 10^(-pOH)M`
We have
`pOH = 1`
For any aqueous solution at 298 K, we have
`pH+pOH=14`
`pH=14-pOH`
`=14-1`
`=13`